sir what about the formal charge of the first oxygen atom? its not 0. i think the best strucure would be a double bond on both sides. correct me if iam wrong.
the creator said that O is more electronegative so you would want the negative charge to go to O, not Cl which would be the case if you did double bonds on both sides
In reality there is something called resonance. So we could draw two lewis structures, one with the double bond on the right and one with it on the left. The actual ClO2 - ion would be an average of the structures. This video for NO2 - might help explain: ruclips.net/video/rrps8QujYA8/видео.html
What is the reason we call HClO3 as chloric acid, not the other ones like HClO4(Perchloric acid) or HClO2(Chlorous acid)? I've seen something like it's decided according to the most general atomic value...? (this is just the translation because I study in Korean) and I just have no idea what "general" means... 😥😥😥
This is just me who is studying chemistry deeply for the first time and it turns out that my textbook is Raymond Chang's general chemistry😭 Too much things to memorize, so it would be sad if I also have to just memorize the oxoacids' names and their formulas 😥😥😥
Yes, there are many things to memorize in chemistry. But there are often general rules (general means broad, typical, common) that can provide some guidance.
Carbon, Nitrogen, Oxygen, and Fluorine do not expand their octets. Chlorine, Sulfur, and certain other elements have the capability to expand their octets to a certain extent, these are exceptions to the rule. Also generally the least electronegative atom goes in the center of a Lewis structure, ClO2 is also an exception of that.
Carbon, Nitrogen, Oxygen, and Fluorine do not expand their octets. Chlorine, Sulfur, and certain other elements have the capability to expand their octets to a certain extent, these are exceptions to the rule. Also generally the least electronegative atom goes in the center of a Lewis structure, ClO2 is also an exception of that.
I use Camtasia Studio to capture the screen and draw in Adobe Illustrator. Often in the video I pause recording to clean things up. It's seems like I'm doing it in real-time to the viewer. The ClO2- Lewis video is an earlier on I did. Take a look at a newer video (ruclips.net/video/ykWLEu9f2Jg/видео.html) where I use Camtasia for some fairly nice post-production effects. Dr. B
O = 3.44, Cl=3.16 blog.prepscholar.com/hs-fs/hubfs/Electronegative.jpg?width=1314&name=Electronegative.jpg But it does seem like it would be, doesn't it?
@@wbreslyn Yeah, I was taught that the electronegativity decreases as you go left on the periodic table, so I assumed Oxygen is more left so it would be less electronegative.
@@ephrataguracha6403 I think of it a F being the most electronegative element. But both O and Cl are next to F so it doesn't help as much there. Just one you have to remember
@@ephrataguracha6403 What? Going toward the right of the periods is where u get more electronegative elements. But some exceptions arise according to electronic configuration such as having a half filled subshell, or fully filled subshell. For example nitrogen has a half filled subshell hence it is less electronegative than oxygen and also bigger in size, and also because oxygen is just towards its right when seen from your perspective. Shielding effect, and so many things matter
+Marcos Fernandes This will help with I3- ruclips.net/video/vlJF_pFtVwU/видео.html I've not done a video for I3 3- but it feels like the extra pair of electrons would go on the central I. You'd have to try it and check the formal charges to see if that makes sense. --- Dr. B
Here you go! Determining Formal Charge: ruclips.net/video/vOFAPlq4y_k/видео.html Formal Charge Practice Video: ruclips.net/video/-9f4H0puVzc-/видео.html-- Dr. B
It's sort of rare to see 10 electrons around Cl. However, Cl is in Period Three on the Periodic Table so it can hold more than 8 valence electrons. It was necessary to have 10 around the Cl in order to make the formal charges as close to zero as possible. --- Dr. B
Wayne Breslyn If your trying to make the formal charge as close to zero as possible, why doesn't Cl have one double bond to each O? That would give a formal charge of zero for each Oxygen. Can you explain?
youkids123 The problem would be that you'd only be using 18 valence electrons, not the 20 we have for the ClO3- lewis structure. If you put put 10 valence electrons on the Cl to use the 20 valence electrons the negative charge would be on the CL. We'd expect to see the negative charge on the more electronegative atom (the Oxygen). It may seem picky but that's the reasoning. --- Dr. B
but if u gain an electron it should be - ? and Cl didn't gain one, it actually binds with one less.It has 7 electrons to bind with, but in the end it only uses 6 of it, thus it is +1. And that makes no sense for me, because we need a charge of minus one! If Cl would bind to O with two double bonds it would use one e more and would have a negative charge. Of course, then it would have more then 8 electrons, but Cl is found in the 3 Period, so that should be okay I guess...this video is confusing :D@@courtneyspencer7297
Stan, you're right! In this case it would just be shifting the double bond to the other side so we'd have two resonance structures for ClO2- (although when we think of resonance it's really an average of the two Lewis structures). Note that the structure earlier in the video with all single bonds is also a resonance structure but not a very important one. ---Dr. B.
Thanks so much for all the time you've taken to put these lewis dot structures up-A College student who is not a fan of chemistry.
Wow, I never understood this during the semester. Now that I am 3 days away from my final I understand it. Thank you so much!!!
Glad it helped and all the best on your final!
lamo i just studying in class 11😂
Me too
@@nishikantsinha2459 bro is from India💀
wow, your teaching style is easy to understand, thank you very much. may god bless you
Thanks and welcome!
Hello! But is not also a valid resonace structure, not necessarily the best, for Cl to have a double bond to each of the oxigens?
this man is saving me from failing research chem
Thank you for the videos man. You're a real hero
You are most welcome!
thnkssss u make this look very easy
sir what about the formal charge of the first oxygen atom? its not 0. i think the best strucure would be a double bond on both sides. correct me if iam wrong.
Yeah true . That is what is written in my yextbook
the creator said that O is more electronegative so you would want the negative charge to go to O, not Cl which would be the case if you did double bonds on both sides
that was so pellucid , thank Doctor
I didn't understand why the double bound. DoesThe double bound moves from one to the other oxygen as the position of the electron is undefined?
In reality there is something called resonance. So we could draw two lewis structures, one with the double bond on the right and one with it on the left. The actual ClO2 - ion would be an average of the structures. This video for NO2 - might help explain: ruclips.net/video/rrps8QujYA8/видео.html
Thank You.
What is the reason we call HClO3 as chloric acid, not the other ones like HClO4(Perchloric acid) or HClO2(Chlorous acid)? I've seen something like it's decided according to the most general atomic value...? (this is just the translation because I study in Korean) and I just have no idea what "general" means... 😥😥😥
This is just me who is studying chemistry deeply for the first time and it turns out that my textbook is Raymond Chang's general chemistry😭 Too much things to memorize, so it would be sad if I also have to just memorize the oxoacids' names and their formulas 😥😥😥
This might help naming acids:
ruclips.net/video/xqHWU5Vj19Q/видео.html
Yes, there are many things to memorize in chemistry. But there are often general rules (general means broad, typical, common) that can provide some guidance.
How exactly can Cl have 10 valence electrons?
Carbon, Nitrogen, Oxygen, and Fluorine do not expand their octets. Chlorine, Sulfur, and certain other elements have the capability to expand their octets to a certain extent, these are exceptions to the rule. Also generally the least electronegative atom goes in the center of a Lewis structure, ClO2 is also an exception of that.
if that's the thing ,then cl could have more than 10 valence electrons , isn't it?
Chlorine only has 7 valence then how can the bonding electrons be 2? isnt it 1?
Carbon, Nitrogen, Oxygen, and Fluorine do not expand their octets. Chlorine, Sulfur, and certain other elements have the capability to expand their octets to a certain extent, these are exceptions to the rule. Also generally the least electronegative atom goes in the center of a Lewis structure, ClO2 is also an exception of that.
@@ChowieWowie In one of the replies the creator said that Cl is more electronegative
Thank you soooo much
Thanks men.
Why are you not using bonds to represent 2 electrons rather than having elements so crunched together? This wasn't taught at all in my Chem lectures
Either way is fine for the bonding electrons. I suppose I left it this way to make sure students understood that a bond is a pair of electrons.
الشكر الجزيل🥰
I LOVE how my chemistry book doesnt mention half of this information. Gotta love modern college. SMH
Sometimes the textbooks are heavy on text but don't give enough examples. The worked examples are probably the best teacher.
Gracias por su explicación
De nada!
why can't we use a dative bond?
how did u calculate non bonding electrons
bruh the electrons which don't take part are non bonding. Where were u looking at 8 years ago?
thank you 💖
No problem! --- Dr. B
Obrigadaa/ thanks!
What kind of program do you use to draw these?
I use Camtasia Studio to capture the screen and draw in Adobe Illustrator. Often in the video I pause recording to clean things up. It's seems like I'm doing it in real-time to the viewer.
The ClO2- Lewis video is an earlier on I did. Take a look at a newer video (ruclips.net/video/ykWLEu9f2Jg/видео.html) where I use Camtasia for some fairly nice post-production effects.
Dr. B
Isn't Oxygen less electronegative than Chlorine?
O = 3.44, Cl=3.16
blog.prepscholar.com/hs-fs/hubfs/Electronegative.jpg?width=1314&name=Electronegative.jpg
But it does seem like it would be, doesn't it?
@@wbreslyn Yeah, I was taught that the electronegativity decreases as you go left on the periodic table, so I assumed Oxygen is more left so it would be less electronegative.
@@ephrataguracha6403 I think of it a F being the most electronegative element. But both O and Cl are next to F so it doesn't help as much there. Just one you have to remember
Wayne Breslyn Got it, thank you!
@@ephrataguracha6403 What? Going toward the right of the periods is where u get more electronegative elements. But some exceptions arise according to electronic configuration such as having a half filled subshell, or fully filled subshell. For example nitrogen has a half filled subshell hence it is less electronegative than oxygen and also bigger in size, and also because oxygen is just towards its right when seen from your perspective. Shielding effect, and so many things matter
Gracias.
De nada!
But why does chlorine go in the middle?!? Chlorine only has one bonding electron. So shouldn't it only be able to bond with one oxygen? not two!!
Chlorine is the least electronegative so therefore it has to go in the middle.
how can i do lewis with I3 3-? and I3 -?
+Marcos Fernandes This will help with I3- ruclips.net/video/vlJF_pFtVwU/видео.html
I've not done a video for I3 3- but it feels like the extra pair of electrons would go on the central I. You'd have to try it and check the formal charges to see if that makes sense. --- Dr. B
+Wayne Breslyn (Dr. B.) Thx!
How to calculate formal charges?
Here you go!
Determining Formal Charge: ruclips.net/video/vOFAPlq4y_k/видео.html
Formal Charge Practice Video: ruclips.net/video/-9f4H0puVzc-/видео.html-- Dr. B
شكرا للإيضاح
لا توجد مشكلة ، يسرني أن أساعد! --- Dr. B
@@wbreslyn
The fact that you went to translate what he said shows how respectable you are. Cheers Brother
Why do you have 10 electrons around CL?
It's sort of rare to see 10 electrons around Cl. However, Cl is in Period Three on the Periodic Table so it can hold more than 8 valence electrons. It was necessary to have 10 around the Cl in order to make the formal charges as close to zero as possible. --- Dr. B
Wayne Breslyn If your trying to make the formal charge as close to zero as possible, why doesn't Cl have one double bond to each O? That would give a formal charge of zero for each Oxygen. Can you explain?
youkids123 The problem would be that you'd only be using 18 valence electrons, not the 20 we have for the ClO3- lewis structure. If you put put 10 valence electrons on the Cl to use the 20 valence electrons the negative charge would be on the CL. We'd expect to see the negative charge on the more electronegative atom (the Oxygen). It may seem picky but that's the reasoning. --- Dr. B
I thought Chlorine couldn’t form double bonds, only Phosphorus, Oxygen, Sulfur, Carbon and Nitrogen?
It is rare but it does happen.
any element below 2nd period can form any bond it wants and exceed the octet rule
Why is there a +1 charge on chlorine?
Jie Long because you gain an electron
but if u gain an electron it should be - ? and Cl didn't gain one, it actually binds with one less.It has 7 electrons to bind with, but in the end it only uses 6 of it, thus it is +1. And that makes no sense for me, because we need a charge of minus one! If Cl would bind to O with two double bonds it would use one e more and would have a negative charge. Of course, then it would have more then 8 electrons, but Cl is found in the 3 Period, so that should be okay I guess...this video is confusing :D@@courtneyspencer7297
thx daddy
When I was teaching high school I had a student who would call me "Uncle" and then my first name. As it was a bit creepy I made him stop. --- Dr. B
U forgot resonance
Stan, you're right! In this case it would just be shifting the double bond to the other side so we'd have two resonance structures for ClO2- (although when we think of resonance it's really an average of the two Lewis structures).
Note that the structure earlier in the video with all single bonds is also a resonance structure but not a very important one.
---Dr. B.
Okay thx
According to my teacher two double bonds is also a valid resonance structure. Do you agree?
Isn’t 7-4-6/2 is -1.5